Cambridge IGCSE Physical Science 0652 — 2009 Oct/Nov Paper 3 · Variant 1

This document consists of 16 printed pages. IB09 11_0652_03/4RP © UCLES 2009 [Turn over *1745915852* For Examiner's Use 1 2 3 4 5 6 7 8 9 Total UNIVERSITY OF CAMBRIDGE INTERNATIONAL EXAMINATIONS International General Certificate of Secondary Education PHYSICAL SCIENCE 0652/03 Paper 3 (Extended) October/November 2009 1 hour 15 minutes Candidates answer on the Question Paper. No Additional Materials are required. READ THESE INSTRUCTIONS FIRST Write your Centre number, candidate number and name on all the work you hand in. Write in dark blue or black pen. You may use a soft pencil for any diagrams, graphs, tables or rough working. Do not use staples, paper clips, highlighters, glue or correction fluid. DO NOT WRITE IN ANY BARCODES. Answer all questions. A copy of the Periodic Table is printed on page 16. At the end of the examination, fasten all your work securely together. The number of marks is given in brackets [ ] at the end of each question or part question. www.XtremePapers.com

2 © UCLES 2009 0652/03/O/N/09 For Examiner's Use 1 (a) A fisherman is steering his boat using a single oar as shown in Fig. 1.1a. Fig. 1.1b shows the same boat viewed from above. To keep the oar stationary the fisherman applies a force of 250 N to the end of the oar. 250 N 2.4 m 0.6 m pivot fisherman Fig. 1a Fig. 1b Calculate the force the oar produces on the water. Show your working. force = [4] (b) The boat moves through the water at a steady speed of 2.5 m / s for 12 s. It then decelerates to rest at a uniform rate in a further 8.0 s. (i) On Fig. 1.2 draw a speed-time graph to show this motion. 0 4 8 12 16 20 3.0 2.0 1.0 0 time / s speed in m / s [2] Fig. 1.2

3 © UCLES 2009 0652/03/O/N/09 [Turn over For Examiner's Use (ii) Calculate the deceleration of the boat. Show your working. deceleration = [2] (iii) Calculate the total distance travelled by the boat. Show your working. distance travelled = [2]

4 © UCLES 2009 0652/03/O/N/09 For Examiner's Use 2 The elements in each group of the Periodic Table show trends in chemical and physical properties. (a) Lithium, sodium and potassium are the first three elements in Group I. (i) Describe the reaction of each element with water to show the trend in the chemical properties of these three elements. [3] (ii) Lithium reacts with water to produce lithium hydroxide and hydrogen. Write a balanced symbol equation for the reaction of lithium with water. [2] (b) Table 2.1 shows information about three elements in Group II. Table 2.1 element atomic number relative atomic mass electron arrangement density in g / cm3 melting point in °C beryllium 4 9 2,2 1.85 1278 magnesium 12 24 2,8,2 1.74 649 calcium 20 40 2,8,8,2 1.54 839 (i) Explain how information in Table 2.1 shows that these three elements are in the same group of the Periodic Table. [2]

5 © UCLES 2009 0652/03/O/N/09 [Turn over For Examiner's Use (ii) The elements in Group II show a trend in physical properties. Use information from Table 2.1 to describe this trend. [2] (iii) Magnesium reacts with chlorine to form magnesium chloride. This compound contains the ions Mg2+ and Cl -. What is the formula of magnesium chloride? [1] (iv) All of the metals in Group II conduct electricity. Use ideas about metallic bonding to explain this fact. [3]

6 © UCLES 2009 0652/03/O/N/09 For Examiner's Use 3 A solar power station is designed for use in desert countries. Fig. 3.1 shows the steps involved in the production of electricity. solar furnace boils water steam drives turbine turbine turns generator generator supplies electricity thermal energy to desalination plant Fig. 3.1 (a) A solar furnace consists of many mirrors. These mirrors are arranged so that sunlight is reflected onto a large container of water, as shown in Fig. 3.2. mirrors water container steam to turbine sunlight Fig. 3.2 (i) Name the process by which the Sun’s energy is transmitted to Earth. [1] (ii) State why the water container is painted black. [1]

7 © UCLES 2009 0652/03/O/N/09 [Turn over For Examiner's Use (iii) Fig. 3.3 shows a ray of sunlight incident on a mirror. Complete the diagram to show the ray after it is reflected from the mirror. mirror normal [1] Fig. 3.3 (b) (i) Name the process by which the energy passes through the wall of the water container. [1] (ii) Explain why the water at the top of the water container is hotter than the water at the bottom of the container. [2] (c) Fig. 3.4 shows the generator. N S output C A B Fig. 3.4 (i) Name part A [1] (ii) Name part B [1]

8 © UCLES 2009 0652/03/O/N/09 For Examiner's Use (iii) Name the material part C is made from, and explain why this material is used. material explanation [2] (d) (i) At the desalination plant thermal energy from the turbine is used to recover pure water from sea water. Name the process by which pure water is recovered from sea water in this desalination plant. [1] (ii) Explain the advantage of combining the desalination plant with the power station. [1]

9 © UCLES 2009 0652/03/O/N/09 [Turn over For Examiner's Use 4 Petroleum contains hydrocarbon molecules with different chain lengths. Long-chain hydrocarbons can be broken down into smaller more useful hydrocarbons. (a) (i) Name the process used to break long-chain hydrocarbons into smaller hydrocarbons. [1] (ii) State an essential condition used in this process and explain why this is used. condition explanation [2] (b) In this process an alkane, C15H32, is broken down. Octane, C8H18, and the alkenes propene, C3H6, and ethene, C2H4, are formed. (i) Write a balanced symbol equation for this reaction. [1] (ii) Describe a chemical test you could use to distinguish between octane and propene. test result for octane result for propene [3] (iii) Ethene can be used to make poly(ethene). State the name of this process. [1] (iv) Propene can be used to make poly(propene). Complete this equation for the formation of poly(propene). n C = C H H H CH3 [2]

10 © UCLES 2009 0652/03/O/N/09 For Examiner's Use 5 Fig. 5.1 shows a circuit diagram, with a battery of e.m.f. of 6.0 V and a resistance wire of length 0.5 m connected across AB. There is a current of 2.4 A in the circuit. 6.0 V 2.4 A A B Fig. 5.1 (a) Calculate the resistance of the resistance wire. resistance = [2] (b) Calculate the power output from the battery. power = [2] (c) (i) The wire is replaced with a wire of the same material and the same diameter but of length1.5 m. Calculate the resistance of this longer wire. resistance = [1] (ii) By making suitable calculations, compare the power output from the battery in (c)(i) with that in (b). [3]

11 © UCLES 2009 0652/03/O/N/09 [Turn over For Examiner's Use 6 Green plants make glucose by the process of photosynthesis. 6CO2 + 6H2O
C6H12O6 + 6O2 (a) From where does the plant obtain the energy needed for this process? [1] (b) For each 20 g of glucose made by the plant, calculate (i) the mass of water used, mass of water = g [3] (ii) the volume, at room temperature and pressure, of oxygen made. (The volume of 1 mole of any gas is 24 dm3 at room temperature and pressure.) volume of oxygen made = unit [3]

12 © UCLES 2009 0652/03/O/N/09 For Examiner's Use 7 Fig. 7.1 shows the results of an experiment to measure the half-life of the isotope phosphorus - 34. 0 5 10 15 time / s 20 25 30 1400 1200 1000 800 600 400 200 0 count rate in counts per second Fig. 7.1 (a) (i) Complete the graph by drawing the best-fit curve. [1] (ii) Use the graph to find the half-life of the isotope. Show your working. half-life = s [2]

13 © UCLES 2009 0652/03/O/N/09 [Turn over For Examiner's Use (b) Phosphorus - 34 decays emitting a β-particle. The equation for this decay is: P 34 15 β 0 –1 S + x y (i) Calculate the value of x. [1] (ii) Calculate the value of y. [1] Please turn over for Question 8.

14 © UCLES 2009 0652/03/O/N/09 For Examiner's Use 8 Fig. 8.1 shows the arrangement of carbon atoms in diamond and graphite. diamond graphite Fig. 8.1 (a) For each of the following properties, compare the two forms of carbon and relate the differences to their structures. (i) melting point [3] (ii) electrical conductivity [3] (b) Graphite burns in oxygen to produce carbon dioxide. (i) Name the type of bonding in carbon dioxide. [1]

15 © UCLES 2009 0652/03/O/N/09 [Turn over For Examiner's Use (ii) Draw a dot and cross diagram to show the arrangement of electrons in carbon dioxide. [3] 9 The Sun and other stars produce energy by nuclear fusion. (a) Explain what is meant by the term nuclear fusion. [2] (b) In a fusion reaction 3.84 x 10-29 kg of mass is released as energy. Calculate the energy released in the reaction. (c = 3 x 108 m / s) Show your working. energy = [3]

16 Permission to reproduce items where third-party owned material protected by copyright is included has been sought and cleared where possible. Every reasonable effort has been made by the publisher (UCLES) to trace copyright holders, but if any items requiring clearance have unwittingly been included, the publisher will be pleased to make amends at the earliest possible opportunity. University of Cambridge International Examinations is part of the Cambridge Assessment Group. Cambridge Assessment is the brand name of University of Cambridge Local Examinations Syndicate (UCLES), which is itself a department of the University of Cambridge. © UCLES 2009 0652/03/O/N/09 Group 140 Ce Cerium 58 141 Pr Praseodymium 59 144 Nd Neodymium 60 Pm Promethium 61 150 Sm Samarium 62 152 Eu Europium 63 157 Gd Gadolinium 64 159 Tb Terbium 65 162 Dy Dysprosium 66 165 Ho Holmium 67 167 Er Erbium 68 169 Tm Thulium 69 173 Yb Ytterbium 70 175 Lu Lutetium 71 232 Th Thorium 90 Pa Protactinium 91 238 U Uranium 92 Np Neptunium 93 Pu Plutonium 94 Am Americium 95 Cm Curium 96 Bk Berkelium 97 Cf Californium 98 Es Einsteinium 99 Fm Fermium 100 Md Mendelevium 101 No Nobelium 102 Lr Lawrencium 103 1 H Hydrogen 1 7 Li Lithium 3 23 Na Sodium 11 24 Mg Magnesium 12 40 Ca Calcium 20 45 Sc Scandium 21 48 Ti Titanium 22 51 V Vanadium 23 52 Cr Chromium 24 55 Mn Manganese 25 56 Fe Iron 26 59 Co Cobalt 27 59 Ni Nickel 28 64 Cu Copper 29 65 Zn Zinc 30 70 Ga Gallium 31 27 Al Aluminium 13 11 B Boron 5 12 C Carbon 6 14 N Nitrogen 7 16 O Oxygen 8 19 F Fluorine 9 28 Si Silicon 14 31 P Phosphorus 15 32 S Sulfur 16 35.5 Cl Chlorine 17 40 Ar Argon 18 20 Ne Neon 10 4 He Helium 2 73 Ge Germanium 32 75 As Arsenic 33 79 Se Selenium 34 80 Br Bromine 35 84 Kr Krypton 36 39 K Potassium 19 88 Sr Strontium 38 89 Y Yttrium 39 91 Zr Zirconium 40 93 Nb Niobium 41 96 Mo Molybdenum 42 Tc Technetium 43 101 Ru Ruthenium 44 103 Rh Rhodium 45 106 Pd Palladium 46 108 Ag Silver 47 112 Cd Cadmium 48 115 In Indium 49 119 Sn Tin 50 122 Sb Antimony 51 128 Te Tellurium 52 127 I Iodine 53 131 Xe Xenon 54 137 Ba Barium 56 139 La Lanthanum 57 * 178 Hf Hafnium 72 181 Ta Tantalum 73 184 W Tungsten 74 186 Re Rhenium 75 190 Os Osmium 76 192 Ir Iridium 77 195 Pt Platinum 78 197 Au Gold 79 201 Hg Mercury 80 204 Tl Thallium 81 207 Pb Lead 82 209 Bi Bismuth 83 Po Polonium 84 At Astatine 85 Rn Radon 86 Fr Francium 87 227 Ac Actinium 89 9 Be Beryllium 4 I II III IV V VI VII 0 85 Rb Rubidium 37 133 Cs Caesium 55 226 Ra Radium 88 The volume of one mole of any gas is 24 dm3 at room temperature and pressure (r.t.p.). a X b a = relative atomic mass X = atomic symbol b = proton (atomic) number Key *58-71 Lanthanoid series 90-103 Actinoid series DATA SHEET The Periodic Table of the Elements

UNIVERSITY OF CAMBRIDGE INTERNATIONAL EXAMINATIONS International General Certificate of Secondary Education MARK SCHEME for the October/November 2009 question paper for the guidance of teachers 0652 PHYSICAL SCIENCE 0652/03 Paper 3 (Extended), maximum raw mark 80 This mark scheme is published as an aid to teachers and candidates, to indicate the requirements of the examination. It shows the basis on which Examiners were instructed to award marks. It does not indicate the details of the discussions that took place at an Examiners’ meeting before marking began, which would have considered the acceptability of alternative answers. Mark schemes must be read in conjunction with the question papers and the report on the examination. • CIE will not enter into discussions or correspondence in connection with these mark schemes. CIE is publishing the mark schemes for the October/November 2009 question papers for most IGCSE, GCE Advanced Level and Advanced Subsidiary Level syllabuses and some Ordinary Level syllabuses. www.XtremePapers.com

Page 2 Mark Scheme: Teachers’ version Syllabus Paper IGCSE – October/November 2009 0652 03 © UCLES 2009 1 (a) (i) Use of clockwise moment (= 250 × 0.6 (= 150)) (1) anticlockwise moment (= f × 2.4) (1) 150 = f × 2.4 (or 250 × 0.6 = f × 2.4, or attempt to equate) (1) f = 63 (62.5) N (1) [4] (note the first 3 marks can be scored in a single line) (if no other mark is scored a clear attempt to calculate a moment OR an attempt to equate clockwise and anticlockwise moments award 1 mark) (b) (i) horizontal line at 2.5 m/s, starting at t = 0, ignore length (1) diagonal line to time axis covering 8 s (1) [2] (ii) attempt to calculate gradient or 2.5 m/s / 8 s (accept ecf) (1) = 0.31 m/s2 (accept m/s/s) (ignore minus signs) (1) [2] (iii) attempt to find area under the graph or (2.5 × 12) + (½ × 2.5 × 8) OR use of s = ut + ½at2 (allow ecf) (1) = 40 m (1) [2] [Total: 10] 2 (a) (i) mention of fizzing/effervescence/hydrogen given off (1) mention of movement across the water or forming a hydroxide (1) increased fizzing/movement down the group/reactivity increases (1) [3] (ii) 2Li + 2H2O
2LiOH + H2 ALL formulae correct (do not allow wrong case for first mark but allow it to qualify for the second mark) (1) one mark for balancing (1) [2] (Li + H2O
LiOH + H give 1 mark) (b) (i) mention of outer shell (1) each has two electrons/same number of electrons (1) [2] (number of electrons/atomic number goes up by 8 each time, 1 mark) (ii) mention of density (1) decreases as atomic number increases/down the group (1) [2] (iii) MgCl2 (1) [1] (iv) metals have lattice of positive ions (1) in a sea of electrons (1) electrons move to carry current (1) [3] (first 2 marks can be scored from a labelled diagram) [Total: 13]

Page 3 Mark Scheme: Teachers’ version Syllabus Paper IGCSE – October/November 2009 0652 03 © UCLES 2009 3 (a) (i) radiation or infra-red/light/electromagnetic waves (1) [1] (ii) black is a good absorber of radiation/energy, etc. (1) [1] (allow, ‘to absorb energy’/radiation, etc.) (iii) ray correctly drawn (1) [1] (b) (i) conduction (1) [1] (ii) hot water less dense than cold/water expands (not molecules) (1) therefore floats/rises to the top (1) [2] (do NOT allow heat rising) (allow 1 mark for mention of convection) (c) (i) slip ring (not split rings) (1) [1] (ii) (carbon) brush (1) [1] (iii) (soft) iron (if more than one answer given – zero, except treat cobalt/ nickel/steel as neutral) (1) increases magnetic field strength/easily magnetised/demagnetised/ acts as an electromagnet (1) [2] (d) (i) distillation (accept evaporation then condensation) (1) [1] (ii) idea that waste energy from turbine is used (1) [1] [Total: 12]

Page 4 Mark Scheme: Teachers’ version Syllabus Paper IGCSE – October/November 2009 0652 03 © UCLES 2009 4 (a) (i) cracking (1) [1] (ii) catalyst OR heat/high temperature (1) increase rate of reaction OR provide energy to break bonds (1) [2] (do NOT allow pick and mix, do not allow ‘break chains’, as in question stem) (b) (i) C15H32
C8H18 + C3H6 + 2C2H4 (1) [1] (ii) add bromine (water); (1) no (colour) change; (+1) (orange/red colour) changes to colourless/decolourises (+1) [3] (iii) (addition) polymerisation [1] (iv) CH3 H H H C C C C H H H CH3 n n one mark lost for each error [2] [Total: 10] 5 (a) use of R = V/I (= 6.0/2.4) (1) = 2.5 Ω (1) [2] (b) use of power = V × I (= 6 × 2.4) (1) = 14.4 W (1) [2] (c) (i) 3 × 2.5 or answer to (a) = 7.5 Ω (1) [1] (ii) attempted calculation of power either by V2 / R or other means (1) = 4.8 W (1) power less with higher resistor or correct conclusion from their figures (1) [3] [Total: 8]

Page 5 Mark Scheme: Teachers’ version Syllabus Paper IGCSE – October/November 2009 0652 03 © UCLES 2009 6 (a) from light/ultra-violet/Sun/sunlight/solar energy (1) [1] (b) (i) C6H12O6 RAM = 180 and/or H2O RAM = 18 (1) 180 g glucose from 108 g water or 108/180 (= 0.6) (1) 20 g glucose from 108 × 20 / 180 = 12 g water (1) [3] (ii) when 180 g glucose is made 6 × 24000 = 14 4000 cm3 oxygen is produced (1) 20 g glucose made with 144000 × 20 / 180 = 16000 (1) cm3 (accept work in dm3) (1) [3] [Total: 7] 7 (a) (i) smooth curve going within 1 square of all points (1) [1] (ii) clear working or 12.5 ± 1.0 s (1) 12.5 ± 0.5 s (1) [2] (when marking final answer, if 12.5 ± 0.5 give 2 marks, 12.5 ± 1.0 for 1 mark) (b) (i) x is 34 (1) [1] (ii) y is 16 (1) [1] [Total: 5] 8 (a) (i) diamond melting point higher than graphite (1) all diamond atoms held by strong (covalent) bonds (1) graphite has fewer bonds to break/weak bonds between layers (1) [3] (ii) diamond does not conduct electricity or graphite does (1) electrons not mobile in diamond (1) graphite has mobile electrons (between layers) (1) [3] (b) (i) covalent [1] (ii) two oxygen atoms each overlapping/‘attached’ to one carbon atom (1) two pairs of electrons in each overlap (1) correct numbers of electrons on both oxygen and the carbon atoms (1) [3] [Total: 10] 9 (a) The joining of two (light) nuclei (do not accept atoms) (1) with release of energy/exothermic reaction (1) [2] (b) Use of E = mc2 (1) = 3.84 × 10–29 × (3 × 108)2 (1) = 3.46 × 10–12 J (1) [3] [Total: 5]